Read the following and answer the question:
Chemistry in Automobiles:
For an internal combustion engine to move a vehicle down the road, it must convert the energy stored in the fuel into mechanical energy to drive the wheels. In your car,the distributor and battery provide this starting energy by creating an electrical "spark", which helps in combustion of fuels like gasoline. Below is the reaction depicting complete combustion of gasoline in full supply of air:
`2C_(8)H_(18)(l) +25O_(2)(g) to 16'X' +Y`
Which of the following are the products obtained from the reaction mentioned in the above case?

Options

A. Product 'X' Product 'Y'
`CO_(2)" " H_(2)O_(2)`
B. Product 'X' Product 'Y'
`H_(2)O" " CO`
C. Product 'X' Product 'Y'
`CH_(3)OH" " H_(2)O`
D. Product 'X' Product 'Y'
`CO_(2) " "H_(2)O`

Explanation

To determine the products obtained from the complete combustion of gasoline (C₈H₁₈), we can follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of octane (C₈H₁₈).
The complete combustion of octane in the presence of oxygen (O₂) produces carbon dioxide (CO₂) and water (H₂O). The unbalanced equation is:
\[ C₈H₁₈ + O₂ \rightarrow CO₂ + H₂O \]

### Step 2: Balance the equation.
To balance the equation, we need to ensure that the number of atoms of each element on the reactant side is equal to the number of atoms on the product side.

1. **Carbon atoms**: There are 8 carbon atoms in C₈H₁₈, so we need 8 CO₂.
2. **Hydrogen atoms**: There are 18 hydrogen atoms in C₈H₁₈, so we need 9 H₂O (since each water molecule has 2 hydrogen atoms).
3. **Oxygen atoms**: Now we need to calculate the total number of oxygen atoms required. From 8 CO₂, we get \(8 \times 2 = 16\) oxygen atoms, and from 9 H₂O, we get \(9 \times 1 = 9\) oxygen atoms. Therefore, we need a total of \(16 + 9 = 25\) oxygen atoms, which means we need \( \frac{25}{2} = 12.5 \) O₂ molecules.

However, since we are given the reaction in terms of whole numbers, we can multiply all coefficients by 2 to eliminate the fraction:
\[ 2C₈H₁₈ + 25O₂ \rightarrow 16CO₂ + 18H₂O \]

### Step 3: Identify the products.
From the balanced equation, we can see that:
- \(X\) corresponds to \(CO₂\) (carbon dioxide).
- \(Y\) corresponds to \(H₂O\) (water).

### Final Answer:
The products obtained from the complete combustion of gasoline (C₈H₁₈) in full supply of air are:
- \(X = CO₂\) (carbon dioxide)
- \(Y = H₂O\) (water)

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